What mass of ammonium chloride must be added to a 0.500 L solution of 0.250 M am

Question

What mass of ammonium chloride must be added to a 0.500 L solution of 0.250 M ammonia to make a buffer with a pH of 9.26? Kb (NH3) = 1.8 x 10-5
What mass of ammonium chloride must be added to a 0.500 L solution of 0.250 M ammonia to make a buffer with a pH of 9.26? Kb (NH3) = 1.8 x 10-5
What mass of ammonium chloride must be added to a 0.500 L solution of 0.250 M ammonia to make a buffer with a pH of 9.26? Kb (NH3) = 1.8 x 10-5
What mass of ammonium chloride must be added to a 0.500 L solution of 0.250 M ammonia to make a buffer with a pH of 9.26? Kb (NH3) = 1.8 x 10-5
What mass of ammonium chloride must be added to a 0.500 L solution of 0.250 M ammonia to make a buffer with a pH of 9.26? Kb (NH3) = 1.8 x 10-5 What mass of ammonium chloride must be added to a 0.500 L solution of 0.250 M ammonia to make a buffer with a pH of 9.26? Kb (NH3) = 1.8 x 10-5

Explanation / Answer

from given realtion we get pH = pKa so [base]/[acid] = 1

0.250*0.5 = 0.125 moles of NH3 = moles of NH4Cl

weight oh ammonium chloride = 0.125*53.4 = 6.675gm

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